1. Write the reaction for the oxidation-reduction performed in this experiment.
ID: 949817 • Letter: 1
Question
1. Write the reaction for the oxidation-reduction performed in this experiment.
2. What oxidation changes does the iron undergo?
3. Why does this oxidation change result in a color change? What color change did you observe?
Please Help!!!
Here is my experiment and results:
Oxidation of Fe2+to Fe3+ 9. Measure and pour 150mL of 3% hydrogen peroxide(H2O2) into the clean 600mL beaker. 10. Use a weigh boat and scale to measure and transfer approximately 3g cream of tartar(KC4HsOs) into the 600mL beaker. 11. Stir the solution with the stir rod until the cream of tartar is evenly distributed throughout the hydrogen peroxide 12. Place the thermometer in the iron acetate solution in the flask and record the initial temperature (Time = 0) in Table 3. 13. Observe and record the color of the iron acetate solution (prepared in Part 1) in Table 3. (1 g of steel wool & 4.5% Acetic Acid, C2H40) 14. Add 15 mL of the iron acetate solution from the flask to the 600 mL beaker. Record the temperature and color of the solution in Table 3 every ten seconds for two minutes; or, until you see a color change take place. You will see a marked increase in temperature as the reaction proceeds. Gently stir the solution as the reaction proceeds. Bubbles should form as carbon dioxide is released.Explanation / Answer
1. The Redox reaction taking place is
Fe2+ (aq.) + H2O2 (aq.) + H2O = Fe2O3 (s) + 4H+ (aq.)
2. Iron undergoes a change from Ferrous (+2) to Ferric (+3) Oxidation State.
3. The initial color change from Clear Brown to Dark Brown is due to formation of Fe3+ ion which complexes with the tartarate present to give a dark brown color. After certain time the color intensity reduces because Ferric Oxide precipitates out of the solution.
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